Can you help with this one? session, mas Mastering Chemistry: Assignment CHM 111

Question

Can you help with this one? session, mas Mastering Chemistry: Assignment CHM 111 K Ch 2 HW Exercise 2.98 Exercise 2.98 Part A Naturally occurring iodine has an atomic mass of Find the apparent "atomic mass" of the contaminated iodine 126.9045. A 12.3849-g sample of iodine is accidentally contaminated with 1.00070 g of L a synthetic Express your answer using six significant figures. radioisotope of iodine used in the treatment of certain diseases of the thyroid gland. The mass of 12 I is 128.9050 amu atomic mass Submit My Answers Give Up

Explanation / Answer

Molar mass of contaminated iodine = Mass total / total moles

Total moles = moles of naturally occurring Iodine + moles of synthetic Iodine

Total mass = 12.3849 g + 1.00070 g

Moles of naturally occurring Iodine =12.3849 g / molar mass of natural Iodine

= 12.3849 g x 1 mol / 126.9045 g

=0.0975923 mol

Moles of synthetic iodine = 1.00070 g x 1 mol / 128.9050 = 0.00776308 mol

Apparent molar mass = ( 12.3849+1.00070)/(0.0975923+0.00776308) =127.05191 amu

So the answer is 127.05191 amu

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